1. What is the volume occupied by 0.248 mol of helium gas at 1.33 atm and 301 K?
2. A cylinder contains 30.5 L of oxygen gas at a pressure of 1.9 atm and a temperature of 288 K. How many moles of gas are in the cylinder?
3.
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An experiment shows that a 256 mL gas sample has a mass of 0.432 g at a pressure of 745 mmHg and a temperature of 28 ∘C. |
What is the molar mass of the gas? |
1) Using ideal gas equation :
V = nRT/P = 0.248×0.082057×301/1.33 L
= 4.6 L
2) n = PV/RT = 1.9×30.5/0.082057×288 moles
= 2.45 moles
3) 760 mmHg = 1atm
745 mmHg = 745/760 atm = 0.98 atm
T = 28°C = 28+273.15 K = 301.15 K
V = 256 ml = 0.256 L
Molar mass = mass×RT/PV
= 0.432×0.082057×301.15/0.98×0.256 g/mol
= 42.55 g/mol
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